CBSE Questions for Class 11 Medical Chemistry Classification Of Elements And Periodicity In Properties Quiz 4 - MCQExams.com

Electronic configuration $$1s^2 2s^2 2px^1 2py^1 2pz^1$$ corresponds to :
  • $$N$$
  • $$Cr$$
  • $$O$$
  • $$F$$
From Be to Ra, ionization energies:
  • increases
  • decreases
  • remain same
  • none of these
There are two elements X and Y. 'X' is the element with the highest $$IP$$ value. 'Y' is the first element in a group possessing strongest reducing property. If X and Y lose 1 and 2 electrons respectively, calculate the $$IP$$ values of the resultant species.
  • 57.2 and 122.4 eV
  • 122.4 eV and 57.2ev
  • 57.2ev and 27. 9 ev
  • None of these
From the following, identify least reactive element:
  • $$_{8}Y^{16}$$
  • $$_{10}Y^{20}$$
  • $$_{11}Y^{23}$$
  • $$_{9}Y^{19}$$
 Which alkali metal element is the most reactive?
  • Caesium
  • Potassium
  • Lithium
  • Francium
The $$100^{th}$$ element is named in honor of:
  • Einstein
  • Bohr
  • Fermi
  • Curie
Structures of nuclei of three atoms A, B, and C are given below-

A has 90 protons and 146 neutrons
B has 92 protons and 146 neutrons
C has 90 protons and 148 neutrons

Based on the above data, which of these atoms are isotopes and which are isobars?
  • A and C are isotopes; B and C are isobars
  • A and B are isotopes; A and C are isobars
  • B and C are isobars; A and B are isobars
  • A and C are isotopes; A and B are isobars
Which of the following order is wrong?
  • $$NH_3< PH_3< AsH_3$$: $$Acidic\ strength$$
  • $$Li< Be<B< C$$: $$IE_1$$
  • $$Al_2O_3< MgO< Na_2O< K_2O$$: $$Basic\ strength$$
  • $$Li^+< Na^+< K^+< Cs^+$$: $$Ionic \:character$$
Ionization potential value of Cs is equal to the electron affinity value of its corresponding __________
  • $$Cs$$
  • $$Cs^+$$
  • $$Cs^2+$$
  • $$Cs^-$$
A neutral atom of an element has a nucleus with nuclear charge $$11$$ times and mass $$23$$ times that of hydrogen. Write the electronic configuration of the element?
  • $$2, 1$$
  • $$2, 8, 1$$
  • $$2, 8$$
  • $$2, 8, 8, 3$$
The numerical value of ionization energy of a unipositive ion is approximately equal to_________
  • IP value of neutral atom.
  • EA value of neutral atom.
  • IP value of dipositive ion.
  • EA value of dipositive ion.
Anomalous pair among the following is:
  • boron - silicon
  • aluminium - nickel
  • beryllium - indium
  • cobalt - nickel
An atom of an element has one electron in the valence shell. It can be represented as :
  • $$_{6}A^{12}$$
  • $$_{19}A^{39}$$
  • $$_{13}A^{27}$$
  • $$_{12}A^{24}$$
The atomic number of Uut is:
  • 113
  • 114
  • 108
  • 115
Which atoms should have smaller value of $$ { \left( IE \right)  }_{ 1 }$$? 

(a) Oxygen or sulphur
(b) Nitrogen or phosphorus
  •  (a) $$S$$ (b) $$P$$
  • (a) $$O$$ (b) $$P$$
  • (a) $$S $$ (b) $$N$$
  • $$None of these$$
A sudden jump between the values of second and third ionization energies of an atom would be associated with the electronic configuration :
  • $${ 1s }^{ 2 },{ 2s }^{ 2 },{ 2p }^{ 6 }{ }^{ }{ }^{ }$$
  • $${ 1s }^{ 2 },{ 2s }^{ 2 }{ 2p }^{ 6 },{ 3s }^{ 2 },{ 3p }^{ 1 }$$
  • $${ 1s }^{ 2 },{ 2s }^{ 2 },{ 2p }^{ 6 },{ 3s }^{ 2 },{ 3p }^{ 2 }$$
  • $${ 1s }^{ 2 },{ 2s }^{ 2 }{ 2p }^{ 6 },{ 3s }^{ 2 }$$
Which of the following pairs show reverse properties on moving along a period from left to right and from top to bottom in a group?
  • Atomic radius and electron gain enthalpy (negative value)
  • Nuclear charge and ionisation enthalpy
  • Ionisation enthalpy and electron gain enthalpy (negative value)
  • None of the above
The nuclear charge actually experienced by an electron is termed as the effective nuclear charge. The effective nuclear charge Z* actually depends on the type of shell and orbital in which electron is actually present. The relative extent to which the various orbitals penetrate the electron clouds of other orbitals is $$s>p>d>f$$ (for the same value of $$n$$)
The phenomenon in which penultimate shell electrons act as screen or shield in between nucleus and valence shell electrons and thereby reducing nuclear charge is known as shielding effect. The penultimate shell electrons repel the valence shell electron to keep them loosely held with the nucleus. It is thus evident that more is the shielding effect, lesser is the effective nuclear charge and lesser is the ionization energy.

Ionization energy is not influenced by :
  • Size of atom
  • Effective nuclear charge
  • Electrons present in inner shell
  • Change in entropy
Which is incorrect configuration for s-block elements?
  • $$[Ar]3d^{10}\, 4s^{2}$$
  • $$[Ar]3d^{10}\, 4s^{1}$$
  • Both A and B
  • None of these
Which is the correct order of ionization energies?
  • $$F^{\displaystyle-}>F>Cl^{\displaystyle-}>Cl$$
  • $$F>Cl>F^{\displaystyle-}>Cl^{\displaystyle-}$$
  • $$F^{\displaystyle-}>Cl^{\displaystyle-}>Cl>F$$
  • $$F^{\displaystyle-}>Cl^{\displaystyle-}>F>Cl$$
Atomic weight of which set of elements were corrected by Mendeleev?
  • $$Li, Na, K$$
  • $$U, Be, In$$
  • $$Tc, Sc, Al$$
  • None of the these
First ionization energy is lowest with :
  • lead
  • carbon
  • silicon
  • tin
The term atomic radius refers to?
  • Charge of the atom
  • Size of the atom
  • Distance between the centre of nucleus and the first shell
  • Size of the outermost orbital
Refer to the Periodic table and identify a highly reactive metal in the sixth period.
  • $$Cs$$
  • $$W$$
  • $$Os$$
  • $$Ir$$
Differentiating electron in $$K(19)$$ goes into ns and this is s-block element. If Aufbau rule is not followed,$$K(19)$$ will be placed in:
  • s-block
  • p-block
  • d-block
  • f-block
Write the electronic configuration of $$Sr^{2+}$$ in absence of Aufbau Principle.
  • $$ 1s^{2},\, 2s^{2}2p^{6},\, 3s^{2}3p^{6}3d^{10},\, 4s^{2}4p^{5}4d^1$$
  • $$ 1s^{2},\, 2s^{2}2p^{6},\, 3s^{2}3p^{6}3d^{10},\, 4s^{2}4p^{3}4d^3$$
  • $$ 1s^{2},\, 2s^{2}2p^{6},\, 3s^{2}3p^{6}3d^{10},\, 4s^{2}4p^{6}$$
  • None of these
Use the following system of naming elements in which first alphabets of the digits are written collectively,
0123456789
nilunibitriquadpenthexseptoctenn
Write three-letter symbol for the elements with atomic number $$106$$.
  • uh
  • unh
  • uunhe
  • unhex
The element $$119$$ has not been discovered. What would be the symbol for this element? 
  • $$Uue$$
  • $$UUe$$
  • $$UUE$$
  • None of these
The single-bonded metallic radius of $$Na$$ is 157 pm. Give a reasonable estimation of the radii, assuming that the increment between radii of different magnitudes is 60 pm. the anionic radius of $$Na$$ is:
  • $$217$$ pm
  • $$227$$ pm
  • $$237$$ pm
  • $$207$$ pm
The electronic configuration of $$Rb^{+}$$ in absence of Aufbau Principle, is:
  • $$1s^{2},\, 2s^{2}2p^{6},\, 3s^{2}3p^{6}3d^{10},\, 4s^{2}4p^{6}$$
  • $$1s^{2},\, 2s^{2}2p^{6},\, 3s^{2}3p^{6}3d^{10},\, 4s^{2}4p^{4}$$
  • $$1s^{2},\, 2s^{2}2p^{6},\, 3s^{2}3p^{6}3d^{10},\, 4s^{2}4p^{3}$$
  • None of these
The factors that influence the ionisation energies are :
  • the size of the atom
  • the charge on the nucleus
  • how effectively the inner electron shell screen the nuclear charge
  • all of the above
Which pair is different from the others?
  • $$Li-Mg$$
  • $$Na-K$$
  • $$Ca-Mg$$
  • $$B-Al$$
The alkalide ion is:
  • diamagnetic
  • represented as $$\overset{-}{C}H_3$$
  • paramagnetic
  • represented as $$\overset{+}{C}H_3$$
Recently (in 2003) element with atomic number $$110$$ has been named by IUPAC as:
  • $$Hs$$
  • $$Mt$$
  • $$Ds$$
  • $$Sg$$
Recently (in Aug 2003) two new elements have been discovered with atomic number:
  • $$113, 114$$
  • $$114, 115$$
  • $$115, 116$$
  • $$113, 115$$
Recently discovered element with atomic number $$ 115$$ is:
  • $$Uun$$
  • $$Uub$$
  • $$Uup$$
  • $$Uus$$
Arrange Be, Ca, Ba, Ra in increasing order of ionisation energy:
  • Be < Ra < Ca < Ba
  • Ba < Ca < Ra < Be
  • Ra < Ba < Ca < Be
  • Ba < Ra < Ca < Be
A hydrogen like ion is an ion containing only one electron. The energies of the electron in a hydrogen like ion are given by $$E_n = - (2.18 \times 10^{-18}) Z^2 \displaystyle \left ( \frac{1}{n^2} \right )$$ joules, where, n is the principal quantum number and Z is the atomic number of the element. Then the ionisation energy (in kJ mol$$^{-1}$$) of the He$$^+$$ ion is:
  • $$2.752 \times 10^3\ kJ mol^{-1}$$
  • $$5.2494 \times 10^3\ kJ mol^{-1}$$
  • $$4.5214 \times 10^3\ kJ mol^{-1}$$
  • $$7.482 \times 10^3\ kJ mol^{-1}$$

Identify the elements in the Periodic Table:

A: Which shows diagonal relationship to $$Be$$

B: Which shows diagonal relationship to $$Li$$
  • $$A : Al , B : Mg$$
  • $$A : Si , B : Mg$$
  • $$A : Mg , B : Al$$
  • $$A : Al , B : Si$$
IE of an element does not depend on :
  • its nuclear charge
  • the shielding effect
  • electron neutrality
  • penetration effect
  • Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
  • Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
  • Assertion is correct but Reason is incorrect
  • Assertion is incorrect but Reason is correct
The element whose electronic conguration is $$1s^22s^22p^63s^2$$ is :
  • non-metal
  • noble gas
  • metalloid
  • metal
State the electronic configuration for Nitrogen [p=7, n=7].
  • 2, 3
  • 2, 4
  • 2, 6
  • 2, 5
State the electronic configuration for Helium [$$p=2,\ n=2$$].
  • $$1$$ 
  • $$3, 2$$
  • $$2$$
  • $$2, 4$$
State the electronic configuration for Potassium [$$p=19,\ n=20$$].
  • $$2, 8, 8, 1$$
  • $$2, 8, 8, 2$$
  • $$2, 8, 8, 3$$
  • $$2, 8, 8, 4$$
State the electronic configuration for Magnesium [p=$$12$$, n=$$12$$].
  • $$2, 8, 0$$
  • $$2, 8, 1$$
  • $$2, 8, 2$$
  • $$2, 8, 3$$
'Electronic configuration' represents :
  • arrangement of protons
  • arrangement of neutrons
  • arrangement of electrons
  • arrangement of electrons, protons and neutrons
Match the statements in List I with the correct answers in list II
List IList II
The basic unit of matterA: Proton
The sub-atomic particle with a positive chargeB: Neon
An atom having stable electronic configurationC: Oxygen
A molecule formed by sharing of electron [covalency]D: Sodium
A metallic atom having unstable electronic configurationE: Atom
  • 1-A, 2-B, 3-C, 4-D, 5-E
  • 1-C, 2-B, 3-A, 4-D, 5-E
  • 1-A, 2-C, 3-B, 4-E, 5-D
  • 1-A, 2-B, 3-D, 4-E, 5-C
  • 1-E, 2-A, 3-B, 4-C, 5-D
State the electronic configuration for Neon [p=10, n=10].
  • 2, 6
  • 2, 7
  • 2, 9
  • 2, 8
What is the electronic configuration of calcium [$$p=20,\ n=20$$]?
  • $$2, 8, 8, 1$$
  • $$2, 8, 8, 3$$
  • $$2, 8, 8, 2$$
  • $$2, 8, 10$$
0:0:1


Answered Not Answered Not Visited Correct : 0 Incorrect : 0

Practice Class 11 Medical Chemistry Quiz Questions and Answers